Subjective Type

What are electron deficient compounds ? Are BCl3 and SiCl4 electron deficient species? Explain.

Solution

In electron deficient compounds, the central atom either does not have eight electrons in the valence shell or it has eight electrons but can expand its valence beyond 4 due to presence of vacant d orbitals.
$$\displaystyle BCl_3 $$ has 6 valence electrons on B atom and accepts pair of electrons from ammonia to complete its octet. Hence, it is an electron deficient compound.
In $$\displaystyle SiCl_4 $$, the central Si atom has 8 electrons but it can expand its valency beyond 4 due to presence of vacant d orbitals. Hence, it is also an electron deficient compound.

SIMILAR QUESTIONS

p - block Elements

Thallous chloride is more stable than Thallic chloride because of

p - block Elements

Anhydrous $$AlCl_{3}$$ is covalent but hydrated $$AlCl_{3}.6H_{2}O$$ is ionic because:

p - block Elements

Which of the following is not an ionic trihalide?

p - block Elements

How can you explain higher stability of BCl3 as compared to TlCl3?

p - block Elements

Aluminium trifluoride is insoluble in anhydrous HF but dissolves on addition of NaF. Aluminium trifluoride precipitates out of the resulting solution when gaseous BF3 is bubbled through. Give reasons.

p - block Elements

BF3 is used as a catalyst in various organic reactions because ?

p - block Elements

Back bonding in $${ BF } _{ 3 }$$ does not affect :

p - block Elements

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p - block Elements

Which of the following statements about anhydrous aluminium chloride is correct?

p - block Elements

Which is true for an element present in group 13 of the periodic table?

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